Podcast
Questions and Answers
What are group 1 elements?
What are group 1 elements?
Alkali metals
What are group 2 elements?
What are group 2 elements?
Alkaline earth metals
What are group 3-12 metals?
What are group 3-12 metals?
Transition metals
What are the elements along the zig-zag or in between the metals and nonmetals?
What are the elements along the zig-zag or in between the metals and nonmetals?
What group is 17 or 7A?
What group is 17 or 7A?
What group is 18 or 8A?
What group is 18 or 8A?
What are the elements at the bottom of the periodic table?
What are the elements at the bottom of the periodic table?
What are metals?
What are metals?
What are the chemical properties of metals?
What are the chemical properties of metals?
What do the group numbers also represent?
What do the group numbers also represent?
What are physical properties of metals?
What are physical properties of metals?
Which metal is not a solid at room temperature?
Which metal is not a solid at room temperature?
Most metals have ___________________ valence electrons. Valence electrons are easily ___________, making some metals ___________________.
Most metals have ___________________ valence electrons. Valence electrons are easily ___________, making some metals ___________________.
All alkali metals have ____ valence electron.
All alkali metals have ____ valence electron.
Alkali metals are _________ found in pure form in nature; they are too ____________.
Alkali metals are _________ found in pure form in nature; they are too ____________.
Reactivity ______________ down the group. Are alkali metals very reactive?
Reactivity ______________ down the group. Are alkali metals very reactive?
What are some physical properties of alkali metals?
What are some physical properties of alkali metals?
All alkaline earth metals have ______ valence electrons.
All alkaline earth metals have ______ valence electrons.
Alkaline earth metals are _______ reactive than alkali metals.
Alkaline earth metals are _______ reactive than alkali metals.
Alkaline earth metals are _____ found in a pure form in nature; they are too _______________.
Alkaline earth metals are _____ found in a pure form in nature; they are too _______________.
What does the word alkaline mean?
What does the word alkaline mean?
What are nonmetals?
What are nonmetals?
What are chemical properties of nonmetals?
What are chemical properties of nonmetals?
What are physical properties of nonmetals?
What are physical properties of nonmetals?
Which nonmetal is liquid at room temperature?
Which nonmetal is liquid at room temperature?
Nonmetals have a __________________________________ valence energy level. Electrons are easily _____________ by elements with nearly full outer energy levels making them very _______________.
Nonmetals have a __________________________________ valence energy level. Electrons are easily _____________ by elements with nearly full outer energy levels making them very _______________.
Halogens have ___ valence electrons. Halogens are the most __________ group of nonmetals. Halogens are only found in a pure form as a ___________ element.
Halogens have ___ valence electrons. Halogens are the most __________ group of nonmetals. Halogens are only found in a pure form as a ___________ element.
Noble gases have ________ valence electrons (full outer energy level) except helium that has _______ valence electrons.
Noble gases have ________ valence electrons (full outer energy level) except helium that has _______ valence electrons.
Noble gases are chemically _________________ and are only found in pure form in nature. They are _____________ and ______________.
Noble gases are chemically _________________ and are only found in pure form in nature. They are _____________ and ______________.
What are the chemical properties of metalloids?
What are the chemical properties of metalloids?
What are the physical properties of metalloids?
What are the physical properties of metalloids?
What do p-block elements contain?
What do p-block elements contain?
P-block and s-block elements make up the __________________ elements.
P-block and s-block elements make up the __________________ elements.
Properties of the p-block __________ greatly.
Properties of the p-block __________ greatly.
Which Russian chemist was the first to publish a system classifying elements in 1869?
Which Russian chemist was the first to publish a system classifying elements in 1869?
What is always the same no matter what language the Periodic Table is published in?
What is always the same no matter what language the Periodic Table is published in?
What did Mendeleev do that finally convinced scientists that his table worked?
What did Mendeleev do that finally convinced scientists that his table worked?
What were two problems with Mendeleev's Periodic Table?
What were two problems with Mendeleev's Periodic Table?
In what order did Mendeleev organize the elements known at his time?
In what order did Mendeleev organize the elements known at his time?
Henry Moseley in 1911 was credited for what three things regarding the periodic table?
Henry Moseley in 1911 was credited for what three things regarding the periodic table?
What is the periodic law?
What is the periodic law?
What does periodically mean?
What does periodically mean?
There are ____ naturally occurring elements.
There are ____ naturally occurring elements.
All elements in the same period have the same number of
All elements in the same period have the same number of
Elements are also arranged vertically in the periodic table in _______ that share similar _________ ______________.
Elements are also arranged vertically in the periodic table in _______ that share similar _________ ______________.
Elements in groups have the same number of ____________ ____________. And therefore lose or gain the same number of electrons when forming ions.
Elements in groups have the same number of ____________ ____________. And therefore lose or gain the same number of electrons when forming ions.
Inner levels of electrons ___________ the outer (valence) electrons blocking the _____________ ______________ on these electrons.
Inner levels of electrons ___________ the outer (valence) electrons blocking the _____________ ______________ on these electrons.
Going down the group, shielding ________________ with the addition of more energy levels.
Going down the group, shielding ________________ with the addition of more energy levels.
The hold on the valence electrons by the _________________ is weakened causing the electrons to become easier to remove.
The hold on the valence electrons by the _________________ is weakened causing the electrons to become easier to remove.
Why is the most reactive nonmetal fluorine?
Why is the most reactive nonmetal fluorine?
What is atomic radius?
What is atomic radius?
How is atomic radius measured?
How is atomic radius measured?
What is the periodic trend of atomic radius?
What is the periodic trend of atomic radius?
The number of protons increasing in the nucleus while going across a period increases the ____________ __________ ___________.
The number of protons increasing in the nucleus while going across a period increases the ____________ __________ ___________.
What does an increase in positive nuclear charge do to an atom?
What does an increase in positive nuclear charge do to an atom?
Moving down a group, each new period adds another energy level. Each level is ____________ from the ______________ and increases the atomic radius.
Moving down a group, each new period adds another energy level. Each level is ____________ from the ______________ and increases the atomic radius.
Positive ions are ___________ than the neutral atom from which they are formed.
Positive ions are ___________ than the neutral atom from which they are formed.
Valence electrons are removed. More protons than electrons cause the _____________ to 'pull' in electrons closer.
Valence electrons are removed. More protons than electrons cause the _____________ to 'pull' in electrons closer.
The resulting cation is smaller than the ______________ atom.
The resulting cation is smaller than the ______________ atom.
Negative ions are ____________ than the neutral atom from which they are formed.
Negative ions are ____________ than the neutral atom from which they are formed.
The extra ___________ produced from the additional electrons cause the ion to ______________.
The extra ___________ produced from the additional electrons cause the ion to ______________.
Valence electrons are added. More electrons than protons cause the ion to __________ due to repulsive forces.
Valence electrons are added. More electrons than protons cause the ion to __________ due to repulsive forces.
What is ionization energy?
What is ionization energy?
What is the periodic trend for ionization energy?
What is the periodic trend for ionization energy?
What is the group trend for ionization energy?
What is the group trend for ionization energy?
Describe first ionization energy.
Describe first ionization energy.
Why is the second ionization energy for sodium so much higher than the first?
Why is the second ionization energy for sodium so much higher than the first?
Why is there a lower ionization energy for elements further down the group?
Why is there a lower ionization energy for elements further down the group?
What is electronegativity?
What is electronegativity?
What is the periodic trend for electronegativity?
What is the periodic trend for electronegativity?
What is the group trend of electronegativity?
What is the group trend of electronegativity?
Why does electronegativity increase across the period?
Why does electronegativity increase across the period?
Which has a smaller atomic radius, Ca or Ca^2+?
Which has a smaller atomic radius, Ca or Ca^2+?
Which has a smaller atomic radius, F or F-?
Which has a smaller atomic radius, F or F-?
What is shielding?
What is shielding?
How many valence electrons in group 17?
How many valence electrons in group 17?
Why does atomic radius decrease going across the period left to right on the periodic table?
Why does atomic radius decrease going across the period left to right on the periodic table?
Are cations or anions larger?
Are cations or anions larger?
Which element is the most electronegative?
Which element is the most electronegative?
Do metals have high electronegativity?
Do metals have high electronegativity?
Study Notes
Group Elements
- Group 1 elements are known as alkali metals.
- Group 2 elements are identified as alkaline earth metals.
- Transition metals, also referred to as B group or D block elements, are located in groups 3-12 and exhibit metallic properties.
- Metalloids are the elements situated along the zigzag line between metals and nonmetals.
Group Characteristics
- Group 17, or 7A, elements are termed halogens.
- Group 18, or 8A, elements are recognized as noble gases.
- The inner transition elements include lanthanides (6th period) and actinides (7th period), classified as f-block elements.
Metals and Their Properties
- Metals are characterized by their ability to lose electrons easily, forming positive ions known as cations.
- They typically have 1 or 2 valence electrons, making them reactive.
- Chemical properties of metals include losing electrons readily, resulting in a positive charge.
- Physical properties include ductility, malleability, high tensile strength, good electrical and thermal conductivity, and typically a shiny luster; most are solid at room temperature, except for mercury.
Reactivity Trends
- Reactivity tends to increase down the group for alkali metals, making them the most reactive group of metals.
- All alkali metals have one valence electron, while alkaline earth metals have two and are less reactive.
Nonmetals and Their Properties
- Nonmetals are elements that tend to gain electrons, forming negative ions or anions.
- They possess nearly full valence energy levels, leading to a tendency to gain electrons, resulting in negative charges.
- Physical properties include being non-ductile, poor conductors of electricity, brittle, and many being gases at room temperature; bromine is the only liquid nonmetal at room temperature.
Halogens and Noble Gases
- Halogens possess 7 valence electrons and are known to be very reactive nonmetals, usually found as diatomic molecules in nature.
- Noble gases have 8 valence electrons, except for helium, which has 2. They are chemically unreactive, colorless, and odorless.
Periodic Table Insights
- Dmitri Mendeleev is credited with the first systematic classification of elements based on atomic mass.
- Mendeleev’s periodic law suggests that properties of elements are periodic functions of their atomic numbers.
- The periodic table consists of 92 naturally occurring elements and organizes elements into periods (rows) and groups (columns).
Atomic Properties
- Atomic radius is defined as half the distance between the nuclei of identical bonded atoms. It decreases across a period and increases down a group due to the increasing nuclear charge.
- Ionization energy represents the energy required to remove an electron from an atom, which generally increases across a period and decreases down a group due to atomic size.
Electronegativity Trends
- Electronegativity measures an atom's ability to attract electrons; it increases across a period and decreases down a group.
- Fluorine is the most electronegative element, while metals typically have low electronegativity due to their tendency to lose electrons.
Ions and Their Sizes
- Cations are smaller than their parent atoms due to the loss of valence electrons and increased nuclear pull.
- In contrast, anions are larger than their parent atoms, as the addition of electrons leads to increased repulsion among electron configurations.
Additional Concepts
- Shielding refers to the effect where inner electrons repel outer electrons, which affects the nuclear force experienced by valence electrons.
- The periodic behavior of elements involves recognizing the trends in reactivity, size, ionization energy, and electronegativity across periods and groups in the periodic table.
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Description
Test your knowledge on the different groups of elements in the periodic table with this quiz. From alkali metals to metalloids, challenge yourself to remember their definitions and properties. Perfect for chemistry students wanting to review essential concepts.
